Metal amides
Metal amides (systematic name metal azanides) are a class of coordination compounds composed of a metal center with amide ligands of the form NR2−. Amido complexes of the parent amido ligand NH2− are rare compared to complexes with diorganylamido ligand, such as dimethylamido. Amide ligands have two electron pairs available for bonding.
![Tris(dimethylamino)aluminium dimer[1]](http://clevelandohioweatherforecast.com//pFad.php?u=http%3A%2F%2Fen.wikipedia.org%2Fwiki%2FFile%3ATris%28dimethylamino%29aluminium_dimer.png)
Geometry and structure
[edit]In principle, the M-NX2 group could be pyramidal or planar. The pyramidal geometry is not observed.
In many complexes, the amido is a bridging ligand. Some examples have both bridging and terminal amido ligands. Bulky amide ligands have a lesser tendency to bridge. Amide ligands may participate in metal-ligand π-bonding giving a complex with the metal center being co-planar with the nitrogen and substituents. Metal bis(trimethylsilyl)amides form a significant subcategory of metal amide compounds. These compounds tend to be discrete and soluble in organic solvents.
Alkali metal amides
[edit]Lithium amides are the most important amides. They are prepared from n-butyllithium and the appropriate amine
- R2NH + BuLi → R2NLi + BuH
The lithium amides are more common and more soluble than the other alkali metal analogs. Potassium amides are prepared by transmetallation of lithium amides with potassium t-butoxide (see also Schlosser base) or by reaction of the amine with potassium, potassium hydride, n-butylpotassium, or benzylpotassium.[2]
The alkali metal amides, MNH2 (M = Li, Na, K) are commercially available. Sodium amide (also known as sodamide) is synthesized from sodium metal and ammonia with ferric nitrate catalyst.[3][4] The sodium compound is white, but the presence of metallic iron turns the commercial material gray.
- 2 Na + 2 NH3 → 2 NaNH2 + H2
Lithium diisopropylamide is a popular non-nucleophilic base used in organic synthesis. Unlike many other bases, the steric bulk prevents this base from acting as a nucleophile. It is commercially available, usually as a solution in hexane. It may be readily prepared from n-butyllithium and diisopropylamine.
Main group amido complexes
[edit]Amido derivatives of main group elements are well developed.[5]
Transition metal complexes
[edit]Early transition metal amides may be prepared by treating anhydrous metal chloride with alkali amide reagents. In some cases, two equivalents of a secondary amine can be used, one equivalent serving as a base:[6]
- MCln + n LiNR2 → M(NR2)n + n LiCl
- MCln + 2n HNR2 → M(NR2)n + n HNR2·HCl
Transition metal amide complexes have been prepared by these methods:[6]
- treating a halide complex with an alkali amide
- deprotonation of a coordinated amine
- oxidative addition of an amine
Amido-ammine complexes
[edit]Highly cationic metal ammine complexes such as [Pt(NH3)6]4+ spontaneously convert to the amido derivative:
- [Pt(NH3)6]4+ ↔ [Pt(NH3)5(NH2)]3+ + H+
Transition metal amides are intermediates in the base-induced substitution of transition metal ammine complexes. Thus, the Sn1CB mechanism for the displacement of chloride from chloropentamminecobalt chloride by hydroxide proceeds via an amido intermediate:[8]
- [Co(NH3)5Cl]2+ + OH− → [Co(NH3)4(NH2)]2+ + H2O + Cl−
- [Co(NH3)4NH2]2+ + H2O → [Co(NH3)5OH]2+
See also
[edit]References
[edit]- ^ Ouzounis, K.; Riffel, H.; Hess, H.; Kohler, U.; Weidlein, J. (1983). "Dimethylaminoalane, H3−nAl[N(CH3)2]n, n = 1, 2, 3 Kristallstrukturen und Molekülspektren". Zeitschrift für anorganische und allgemeine Chemie. 504 (9): 67–76. doi:10.1002/zaac.19835040909.
- ^ Michael Lappert, Andrey Protchenko, Philip Power, Alexandra Seeber (2009). "2. Alkali Metal Amides". Metal Amide Chemistry. John Wiley & Sons. ISBN 978-0-470-74037-8.
{{cite book}}: CS1 maint: multiple names: authors list (link) - ^ Bergstrom, F. W. (1955). "Sodium Amide". Organic Syntheses; Collected Volumes, vol. 3, p. 778.
- ^ Greenlee, K. W.; Henne, A. L.; Fernelius, W. Conard (1946). "Sodium Amide". Inorganic Syntheses. Vol. 2. pp. 128–135. doi:10.1002/9780470132333.ch38. ISBN 978-0-470-13233-3.
{{cite book}}:|journal=ignored (help) - ^ Waggoner, K.M.; Olmstead, M.M.; Power, P.P. (1990). "Structural and spectroscopic characterization of the compounds [Al(NMe2)3]2, [Ga(NMe2)3]2, [(Me2N)2Al{μ-N(H)1-Ad}]2 (1-Ad = 1-adamantanyl) and [{Me(μ-NPh2)Al}2NPh(μ-C6H4)]". Polyhedron. 9 (2–3): 257–263. doi:10.1016/S0277-5387(00)80578-1.
- ^ a b John F. Hartwig (2009). "4. Covalent (X-Type) Ligands Bound Through Metal-Heteroatom Bonds". Organotransition Metal Chemistry: From Bonding to Catalysis. University Science Books. ISBN 978-1-891389-53-5.
- ^ Curley, J. J.; Cook, T. R.; Reece, S. Y.; Müller, P.; Cummins, C. C. (2008). "Shining Light on Dinitrogen Cleavage: Structural Features, Redox Chemistry, and Photochemistry of the Key Intermediate Bridging Dinitrogen Complex". Journal of the American Chemical Society. 130 (29): 9394–9405. doi:10.1021/ja8002638. PMID 18576632.
- ^ G. L. Miessler and D. A. Tarr "Inorganic Chemistry" 3rd Ed, Pearson/Prentice Hall publisher, ISBN 0-13-035471-6.